Can oxygen form an expanded octet?

Atoms with an expanded octet Phosphorous often has 5 orbitals (10 electrons) and sulfur often has 6 orbitals (12 electrons) because they are in the third period, but nitrogen and oxygen can never have expanded octets because they are in the second period and there is not such thing as a 2d orbital.

Why can sulfur Form 6 bonds while oxygen can t?

Sulphur has 6 Valance electrons so according to VBT it can form maximum of 6 covalent bonds. Same is with Oxygen but that can form maximum of 3 covalent bonds. This is because of availablity of vacant d orbitals in Sulphur, which can accommodate extra electrons other than octet. Thus sulphur forms SF6.

Can sulfur form an expanded octet?

The octet rule can be ‘expanded’ by some elements by utilizing the d-orbitals found in the third principal energy level and beyond. Sulfur, phosphorus, silicon, and chlorine are common examples of elements that form an expanded octet.

Why can sulfur form more bonds than oxygen?

Originally Answered: why can sulfur form 6 bonds while oxygen can’t? Sulfur is larger and can form an “expanded valence shell”. More specifically, the valence electrons in sulfur are in the 3rd shell, which has unoccupied d orbitals.

Why does sulfur not follow the octet rule?

Here the sulfur atom has six electron pairs in its valence shell. An atom like phosphorus or sulfur which has more than an octet is said to have expanded its valence shell. Expansion of the valence shell is impossible for an atom in the second period because there is no such thing as a 2d orbital.

Which element Cannot have an expanded octet?

These elements include hydrogen, helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine and neon. Elements that cannot have an expanded octet are: hydrogen, helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine and neon.

Why does sulfur exist as s8 and not s2?

Probably because Sulfur forms single bonds rather than double bonds as an element. It forms Pπ bonds. Sulfur (and Selenium also in the same group) due to its bigger atomic size has stronger Vander Waal forces among atoms. So it forms a solid structure at room temperature.

Which compound does not show expanded octet?

Phosphorus pentachloride (PCl5) and sulfur hexafluoride (SF6) are examples of molecules that deviate from the octet rule by having more than 8 electrons around the central atom.

Which elements Cannot have an expanded octet?

What are the differences between sulphur and oxygen?

Sulfur is less electronegative than oxygen (2.4 and 3.5, respectively) and as a consequence bonds to sulfur are less polar than the corresponding bonds to oxygen. One significant result in that with a less polar S-H bond the subsequent hydrogen bonding is weaker than observed with O-H analogs.

Why does sulfur have a larger atomic radius than oxygen?

Sulfur has more electrons and hence more filled atomic orbitals than oxygen. More filled orbital electrons take up more space (due to interatomic electron-electron repulsions)… hence its atomic size is bigger than that of oxygen.

What elements are able to form expanded octets?

Sulfur, phosphorus, silicon, and chlorine are common examples of elements that form an expanded octet. Phosphorus pentachloride (PCl5) and sulfur hexafluoride (SF6) are examples of molecules that deviate from the octet rule by having more than 8 electrons around the central atom.

Does nitrogen follow the octet rule?

Nitrogen generally follows the octet rule. The octet rule is a helpful guide to understanding nitrogen chemistry. There are some notable nitrogen-based molecules that violate this rule. Typically, elements in the first two rows of the periodic table form compounds in accordance with the octet rule.

What is an exception to the octet rule?

The most common exception to the octet rule is a molecule or an ion with at least one atom that possesses more than an octet of electrons. Such compounds are found for elements of period 3 and beyond.

Do noble gases have full octet of electrons?

The noble gases are the only non-transition-metal elements that have eight valence electrons in their neutral, ground state configuration, but atoms of other elements can produce a full octet — an outer shell with eight electrons — by gaining or losing electrons.